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(A) In the given reaction: $P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$The oxidation state of phosphorus $(P)$ in $P_4$ is $0$.In $PH_3$,th

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for disproportionation reaction.

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(A) In the given reaction: $P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$The oxidation state of phosphorus $(P)$ in $P_4$ is $0$.In $PH_3$,the oxidation state of $P$ is $-3$ (reduction).In $NaH_2PO_2$,the oxidation state of $P$ is $+1$ (oxidation).Since the same element $(P)$ is simultaneously oxidized and reduced in the same reaction,this is a disproportionation reaction.Therefore,the correct option is $A$.

Assign $A$,$B$,$C$,$D$ from the given type of reaction.
$P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$
(Note: The reaction provided is the standard balanced equation for the disproportionation of white phosphorus.)

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Assign $A$,$B$,$C$,$D$ from the given type of reaction.$P_4 + 3NaOH + 3H_2O \longrightarrow PH_3 + 3NaH_2PO_2$(Note: The reaction provided is the standard balanced equation for the disproportionation of white phosphorus.)